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Bio 181 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

What are organisms composed of?

A

Organisms are composed of matter.

Matter is anything that takes up space and has mass.

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2
Q

What is matter made up of?

A

Matter is made up of elements, which are anything you can touch, feel, or see.

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3
Q

What are atoms?

A

Atoms are the building blocks of all substances.

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4
Q

What are the components of an atom?

A

Atoms are made of electrons, protons, and neutrons.

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5
Q

What is the interaction between electrons and protons?

A

Electrons and protons pull together, while protons push away from each other.

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6
Q

What defines the element of an atom?

A

The number of protons in the atomic nucleus defines the element.

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7
Q

What defines the isotope of an atom?

A

The number of neutrons defines the isotope.

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8
Q

What is the charge of electrons?

A

Electrons have a negative charge.

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9
Q

What does the nucleus of an atom contain?

A

The nucleus contains protons, which have a positive charge, and neutrons, which have no charge.

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10
Q

What determines the differences in atoms?

A

Differences in atoms can be the number of protons, the number of neutrons, and the number of electrons.

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11
Q

What does atomic number represent?

A

Atomic number (number of protons) determines the element.

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12
Q

What is mass number?

A

Mass number (atomic mass) is the total number of protons and neutrons in a nucleus.

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13
Q

What is mass number used for?

A

Mass number is used to identify isotopes.

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14
Q

What is the periodic table of the elements?

A

An arrangement of the elements based on their atomic number and chemical properties.

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15
Q

What does the periodic table show?

A

It shows how each element is like, how they behave, and how they work with other elements.

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16
Q

What is atomic number?

A

The number of protons in an element.

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17
Q

How is atomic mass calculated?

A

Atomic mass = Protons + Neutrons.

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18
Q

What are isotopes?

A

Different versions of the same element, with different numbers of neutrons.

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19
Q

Can elements have different atomic masses?

A

Yes, but they must have the same atomic number to be a specific element.

Example: Carbon is C, not 5.

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20
Q

What are radioisotopes?

A

Radioactive isotopes that emit subatomic particles or energy when their nucleus breaks down, transforming one element into another at a constant rate.

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21
Q

What is the stability of radioisotopes?

A

They are unstable and give off tiny bits of energy when trying to become stable, known as radiation.

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22
Q

What moves around the nucleus in orbitals?

A

Electrons move around the nucleus in orbitals.

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23
Q

What does each orbital correspond to?

A

Each orbital corresponds to an energy level.

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24
Q

Under what condition can an electron move?

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A

An electron can move only if there is a vacancy.

25
How do electrons move to higher or lower shells?
Electrons move to higher or lower shells by absorbing or releasing energy.
26
What does the shell model of electron orbitals diagram?
The shell model diagrams electron vacancies filled from inside out.
27
How many electrons can the first shell hold?
The first shell can hold 2 electrons.
28
How many electrons can the second shell hold?
The second shell can hold 8 electrons.
29
How many electrons can the third shell hold?
The third shell can hold 6 electrons.
30
What do atoms with vacancies in their outer shell tend to do?
Atoms with vacancies in their outer shell tend to give up, acquire, or share electrons.
31
What is a free radical?
A free radical is an atom with an unpaired electron.
32
What are ions?
Ions are atoms with a positive or negative charge due to the loss or gain of electrons in their outer shell. ## Footnote Examples include Na+ and Cl-.
33
What charge does Na+ have?
Na+ has a +1 charge.
34
What charge does Cl- have?
Cl- has a -1 charge.
35
What do atoms with no charge prefer?
Atoms with no charge would rather give up an electron to have a stronger shell.
36
What do atoms with a negative charge prefer?
Atoms with a negative charge would rather gain an electron to have a full shell.
37
What is a chemical bond?
A chemical bond is an attractive force existing between two atoms when their electrons interact.
38
What is a molecule?
A molecule is two or more atoms joined in chemical bonds.
39
What are compounds?
Molecules consisting of two or more elements whose proportions do not vary. ## Footnote Example: Water (H2O) = Hydrogen atoms + Oxygen atoms.
40
What is a mixture?
Two or more substances that intermingle but do not bond, with varying proportions of each. ## Footnote Example: Trail Mix.
41
What determines whether one atom will bond with others?
It depends on the element and the number and arrangement of its electrons.
42
What is electronegativity?
A measure of the ability of an atom to attract electrons away from other atoms.
43
Why are some atoms more electronegative than others?
Smaller atoms tend to hold onto electrons better, and the number of protons (p+) means a stronger pull on the electrons.
44
What is an ionic bond?
A strong mutual attraction between two oppositely charged ions with a large difference in electronegativity, where no electron is transferred. ## Footnote Example: Table Salt (NaCl) or MgO.
45
What are compounds formed by ionic bonds called?
Ionic compounds.
46
How would you describe a weak chemical bond?
A bond that is not as strong as ionic or covalent bonds.
47
What is a covalent bond?
A covalent bond is formed when two atoms with similar electronegativity and unpaired electrons share a pair of electrons.
48
How do covalent bonds compare to ionic bonds?
Covalent bonds can be stronger than ionic bonds.
49
How many pairs of electrons can atoms share in covalent bonds?
Atoms can share one, two, or three pairs of electrons, forming single, double, or triple covalent bonds.
50
What is a non-polar covalent bond?
A non-polar covalent bond is formed when atoms share electrons equally, typically between atoms with identical electronegativity. ## Footnote Example: O2
51
What is polarity in the context of covalent bonds?
Polarity refers to the separation of charge into distinct positive and negative regions in a polar covalent molecule. ## Footnote Example: Water
52
What is a polar bond?
Atoms with different electronegativity, do not share electrons equally; one atom has more negative charge, the other is more positive Example: Water, H2O
53
What is the overall charge of water (H2O)?
Water (H2O) has no charge, but it is polar.
54
What is the charge of the oxygen and hydrogen atoms in water?
The oxygen atom is slightly negative, while the hydrogen atoms are slightly positive.
55
What is a hydrogen bond?
A hydrogen bond is a weak attraction between a highly electronegative atom and a hydrogen atom participating in a separate polar covalent bond.
56
Do hydrogen bonds form molecules?
No, hydrogen bonds do not form molecules and are not chemical bonds.
57
What do hydrogen bonds stabilize?
Hydrogen bonds stabilize the structures of large biological molecules.
58
What are some properties of water?
Water has cohesive behavior, the ability to moderate temperature, expansion upon freezing, and versatility as a solvent.

Bio 181 (2 decks)

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